Additional Homework for Chp. 2.
4. Calculate the final temperature of a sample of CO2 of mass 16.0g that is expanded
reversibly and adiabatically from 500.0mL at 298K to 2.00L.
Additional Homework for Chp. 3
1. Calculate the maximum efficiency of
a) a primitive steam engine (cyclical heat engine) operating on steam at 100o C and
discharging at 60o C.
b) a more modern steam turbine that operates with steam at 300o C and discharges at
80o C.
2. Calculate the change in entropy when 25 kJ of energy is transferred reversibly and
isothermally as heat to a large block of iron at 0o C.
3. A sample consisting of 1.00 mol of a monatomic perfect gas with Cvm = 3/2 R is heated
from 0o C to 100o C at constant pressure. Calculate S for the system.
4. Calculate S for the system when the state of 3.00 mol of a monatomic perfect gas, for
which Cp,m = 5/2 R, is changed from 25o C and 1.00 atm to 125o C and 5.00 atm.
Rationalize the sign of S.
5. A sample consisting of 3.00 mol of a diatomic perfect gas at 200.K is compressed
reversibly and adiabatically until its temperature reaches 250.K. Given that Cvm = 27.5
J/(mol K), calculate q, w, U, H, and S.
6. Calculate the change in the entropies of the system and the surroundings and the total
change in entropy, when the volume of a sample of nitrogen gas of mass 14 g at 298K
and 1.0 bar doubles its volume in an
a) isothermal reversible expansion
b) isothermal Irreversible expansion against Pex = 0.
c) adiabatic reversible expansion
7. Calculate the change in entropy when a monatomic perfect gas is compressed to half
its volume of 2.00L and simultaneously heated to twice its initial temperature of 300K.
Assume Cvm = 3/2R.